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Structure and bonding - Coggle Diagram

- - - - Contain regular structures (giant ionic lattices) - strong forces of attraction in all directions due to oppositely charged ions
      - High melting and boiling points due to the high energy required to break the many strong ionic bonds in all directions
      - When melted or dissolved in water, ionic compounds conduct electricity because ions are free to move and carry current
  - - - Solids that are very hard with extremely high melting and boiling points due to the high energy required to overcome strong covalent bonds between all atoms
      - Many atoms linked to one another by strong covalent bonds
      - Examples of giant covalent structures
        
        Diamond
        
        No delocalised electrons
        
        Cannot conduct electricity
        
        High mpt and bpt - also very hard due to rigid covalent structure
        
        Graphite
        
        Can conduct electricity due to delocalised electrons between layers of graphite that are free to move along
        
        Contains layers of covalently bonded carbon atoms - no bonds between the layers meaning they slide over one another, making graphite a very soft structure
    - - Low melting and boiling points due to the weak intermolecular forces between the molecules requiring low energy to break
      - Intermolecular forces increase with the size of the molecule so larger molecules have higher melting and boiling points
- - - - Cylindrical fullerens with high length to diameter ratios
      - This makes them useful for nanotechnology and electronics
    - - Spherical fullerenes used as lubricants